Two elements 1 and 2 are in the same row of the periodic table but not next to each other. Element 1 has a larger atomic radius than element 2, which of the following are most likely to be true about their relative ionization energies and why? 1. Element 1 has a larger ionization energy 2. Element 2 has a larger ionization energy 3. They both have the same ionization energy Because 1. electrons in element 1 are more strongly attracted to the nucleus 2. electrons in element 2 are more strongly attracted to the nucleus 3. electrons are being removed from the same quantum shell O O O O O 1,3 O 2,3 O 3,2 O 3,3

Two elements 1 and 2 are in the same row of the periodic table but not next to each other. Element 1 has a larger atomic radius than element 2, which of the following are most likely to be true about their relative ionization energies and why? 1. Element 1 has a larger ionization energy 2. Element 2 has a larger ionization energy 3. They both have the same ionization energy Because 1. electrons in element 1 are more strongly attracted to the nucleus 2. electrons in element 2 are more strongly attracted to the nucleus 3. electrons are being removed from the same quantum shell O O O O O 1,3 O 2,3 O 3,2 O 3,3

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter6: The Periodic Table And Atomic Structure

Section: Chapter Questions

Problem 6.82PAE: 6.82 A particular element has the following values for its first four ionization energies: 900,...

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What is the difference between core electrons and valence electrons? Why do we emphasize the valence electrons in an atom when discussing atomic properties? What is the relationship between valence electrons and elements in the same group of the periodic table?
Answer the following questions about first ionization energies. (a) Generally ionization energies increase on proceeding across a period, but this is not true for magnesium (738 kJ/mol) and aluminium (578 kJ/mol). Explain this observation. (b) Explain why the ionization energy of phosphorus (1012 kJ/mol) is greater than that of sulphur (1000 kJ/mol) when the general trend in ionization energies in a period would predict the opposite.
The magnet in the following photo is made from neodymium, iron, and boron. A magnet mode of on alloy containing the elements Nd, Fe, and B. (a) Write the electron configuration of each of these elements using an orbital box diagram and noble gas notation. (b) Are these elements paramagnetic or diamagnetic? (c) Write the electron configurations of Nd3+ and Fe3+ using orbital box diagrams and noble gas notation. Are these ions paramagnetic or diamagnetic?
r Questions 11—13, you will need to consider ionizations beyond the first ionization energy. For example, the second ionization energy is the energy to remove a second electron from an element. Compare the first ionization energy of helium to its second ionization energy, remembering that both electrons come from the 1s orbital. l> X Y First 170 200 second 350 400 Third 1800 3500 fouth 2500 5000 entify the elements X and Y. There may be more than one answer. so explain completely.
Compare the elements Na, Mg, O, and P. (a) Which has the largest atomic radius? (b) Which has the most negative electron attachment enthalpy? (c) Place the elements in order of increasing ionization energy.
6.82 A particular element has the following values for its first four ionization energies: 900, 1760, 14, 850, and 21,000 kJ/mol. Without consulting a list of ionization energy values, determine what group in the periodic table this element belongs in.
Write the symbol of each element described below. (a) largest atomic radius in Group 1 (b) smallest atomic radius in period 3 (c) largest first ionization energy in Group 2 (d) most electronegative in Group 16 (e) element(s) in period 2 with no unpaired p electron (f) abbreviated electron configuration is [Ar] 4s23d3 (g) A +2 ion with abbreviated electron configuration [Ar]3d5 (h) A transition metal in period 4 forming a +2 ion with no unpaired electrons
What main group in the periodic table has elements with the largest electron affinities for each period? What group of elements has only unstable negative ions?
Which ion with a +1 charge has the electron configuration 1s22s22p63s23p63d104s24p6? Which ion with a —2 charge has this configuration?
The following shapes each represent an orbital of an atom in a hypothetical universe. The small circle is the location of the nucleus in each orbital. a If you placed an electron in each orbital, which one would be higher in energy? b When an electron makes a transition from the orbital represented on the right to the orbital on the left, would you expect energy to be absorbed or released? c Draw a sketch of an orbital of the same type that would be higher in energy than either of the two pictured orbitals.
6.84 Which graph correctly depicts the first ionization energy of three elements in groups 14 (dashed line) and 17 (solid line)? Explain the reasoning you used to make your choice.
6.69 Compare the elements Na, B, Al, and C with regard to the following properties. (a) Which has the largest atomic radius? (b) Which has the most negative electron affinity? (c) Place the elements in order of increasing ionization energy.

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